Chemistry
Chemistry, 06.08.2019 05:10, alexsk6357

What is the value of kp for the reaction of nitrogen and oxygen to make dinitrogen monoxide if the equilibrium partial pressures of nitrogen is 1.3241 atm, the partial pressure of oxygen is 1.0844 atm and the partial pressure of dinitrogen monoxide is 0.0339 atm?

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Chemistry, 24.06.2019 18:00, LunaShiner
Nitrogen forms a surprising number of compounds with oxygen. a number of these, often given the collective symbol nox(for "nitrogen + oxygens") are serious contributors to air pollution. they can often be interconverted, sometimes by reaction with oxygen or ozone (o3) in the air. an atmospheric scientist decides to study the reaction between nitrogen dioxide and oxygen that produces dinitrogen pentoxide. he fills a stainless steel reaction chamber with of 2.1 atm nitrogen dioxide gas and 6.7 atm of oxygen gas and raises the temperature considerably. at equilibrium he measures the mole fraction of dinitrogen pentoxide to be 0.10 . calculate the pressure equilibrium constant kp for the equilibrium between nitrogen dioxide, oxygen, and dinitrogen pentoxide at the final temperature of the mixture. round your answer to 2 significant digits.
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Chemistry, 02.08.2019 23:30, montgomerykarloxc24x
Nitrogen forms a surprising number of compounds with oxygen. a number of these, often given the collective symbol (for "nitrogen + oxygens") are serious contributors to air pollution. they can often be interconverted, sometimes by reaction with oxygen or ozone () in the air. an atmospheric scientist decides to study the reaction between nitrogen dioxide and oxygen that produces dinitrogen pentoxide. he fills a stainless steel reaction chamber with of nitrogen dioxide gas and of oxygen gas and raises the temperature considerably. at equilibrium he measures the mole fraction of dinitrogen pentoxide to be . calculate the pressure equilibrium constant for the equilibrium between nitrogen dioxide, oxygen, and dinitrogen pentoxide at the final temperature of the mixture. round your answer to significant digits.
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Chemistry, 14.09.2019 11:10, 1991987
Given the following data at a certain temperature, 2n2(g) + o2(g) + 2n2o(g) k=1.2 x 10-35 n204(g) + 2no2(g) k=4.6 x 10-3 12 n2(g) + o2 + no2(g) k-4.1 x 109 calculate k for the reaction between one mole of dinitrogen oxide gas and oxygen gas to give dinitrogen tetroxide gas. 7. for the system pcls(g) + pc13(g) + cl2(g) k is 26 at 300°c. in a 5.0-l flask, a gaseous mixture consists of all three gases with partial pressure as follows: ppcis = 0.012 atm, pcl2 = 0.45 atm, ppci3 = 0.90 atm. a) is the mixture at equilibrium? explain. b) if it is not at equilibrium, which way will the system shift to establish equilibrium? 8. for the reaction: n2(g) + 2h2o(g) + 2no(g) + 2h2(g) k is 1.54 x 10-3. when equilibrium is established, the partial pressure of nitrogen is 0.168 atm, and that of no is 0.225 atm. the total pressure of the system at equilibrium is 1.87 atm. what are the equilibrium partial pressures of hydrogen and steam?
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